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4 years ago

A gas occupies 4.00 L at 2.00 atm pressure. At what pressure would the volume be 6.00 L if the temperature remains constant?

Chemistry

2 answers:

kherson [118]4 years ago

8 0

P1V1= P2V2
P1= 2
V1=4
V2=6
answere= (8/6)

True [87]4 years ago

6 0

Answer:

The final pressure would be 1.33 atm

Explanation:

Given:

Initial volume of the gas, V1 = 4.00 L

Initial pressure, P1 = 2.00 atm

Final volume, V2 = 6.00 L

To determine:

The final pressure P2 of the gas

Explanation:

Based on the ideal gas equation:

$PV = nRT$

where: n = number of moles,

R = gas constant and T = temperature

At constant Temperature the gas law reduces to,

$PV = constant\\\\P1V1 = P2V2\\\\P2 = \frac{P1V1}{V2} = \frac{2.00atm*4.00L}{6.00L} =1.33\ atm$

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3 years ago

The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCl (aq)) in 133 mL of water is ___ M (2 decimal

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The molarity is 3.50 M/L.

Explanation:

Molarity is found to know the amount of the solute ions present in the given volume of solution. So we determine it using the ratio of the moles of solute to the volume of the solution.

As here the weight of the solute which is hydrochloric acid is given as 17g, so we need to find the moles of it. This can be done by dividing the given amount of HCl with the molecular weight of HCl.

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4 years ago